0.1 M formic acid solution is titrated against 0.1 M NaOH solution. What would be the difference in pH between 1/5 and 4/5 stages of neutralization of acid?
10 mLof H,A (weak diprotic acid) solutions is titrated against 0.1M NaOH. pH of the solution is plotted against volume of strong base added and following observation is made. If pH of the solution at 1^(st) equivalence point is pH_(1) and at 2^(nd) equivalnee point is pH_(2) , Cal the value (pH_(2),-pH_(1)) at 25^(@) C. Given for H_(2),A, p^(Kal) =4.6 &p^(Ka2) =8
100 ml 0.1 M H_3PO_4 solution is being titrated with 0.1 M NaOH solution. The pH of the reaction mixture keeps increasing with addition of NaOH. The successive dissociation constant of H_3PO_4 " are " 10^(-3) , 10 ^(-6) and 10^(-14) respectively. What is the pH of the solution after adding 150 ml of NaOH solution?
100 ml 0.1 M H_3PO_4 solution is being titrated with 0.1 M NaOH solution. The pH of the reaction mixture keeps increasing with addition of NaOH. The successive dissociation constant of H_3PO_4 " are " 10^(-3) , 10 ^(-6) and 10^(-14) respectively. What is the pH of the reaction mixture after adding 50 ml of NaOH ?
100 ml 0.1 M H_3PO_4 solution is being titrated with 0.1 M NaOH solution. The pH of the reaction mixture keeps increasing with addition of NaOH. The successive dissociation constant of H_3PO_4 " are " 10^(-3) , 10 ^(-6) and 10^(-14) respectively. How much volume of the given NaOH must be added such that a buffer H_2PO_4^(-) // HPO_4^(-2) of maximum capacity is formed.
A 25.0ml sample of 0.1 M HCl is titrated with 0.1 M NaOH . What is the pH of the solution at the points where 24.9 and 25.1 ml of NaOH have been added ?
29.5mg of an organic compound containing nitrogen was digested according to Kjeldahl's method and the evolved ammonia was absorbed in 20mL of 0.1M HCl solution. The excess of the acid required 15mL of 0.1M NaOH solution for complete neutralization. The percentage of nitrogen in the compound is
NARENDRA AWASTHI-IONIC EEQUILIBRIUM-Assertin-Reason Type Questions
